Medium
Rate of reaction for $2X + Y \rightarrow 3W + Z$ is $1.2 \times 10^{-4} \ mol \ dm^{-3} \ sec^{-1}$ when $[X] = [Y] = 0.6 \ mol \ dm^{-3}$. Calculate the value of the rate constant if the reaction is first order in $X$ and zero order in $Y$.
- A$2 \times 10^{-4} \ sec^{-1}$
- B$6 \times 10^{-3} \ mol \ dm^{-3} \ sec^{-1}$
- C$4 \times 10^{-4} \ sec^{-1}$
- D$1.8 \times 10^{-3} \ mol \ dm^{-3} \ sec^{-1}$
Explore More
Similar Questions
For the non-stoichiometric reaction $2A + B \to C + D$,the following kinetic data were obtained in three separate experiments,all at $298 \ K$.
Initial Conc. $(A)$ Initial Conc. $(B)$ Initial rate of formation of $C \ (mol \ L^{-1} \ s^{-1})$ $0.1 \ M$ $0.1 \ M$ $1.2 \times 10^{-3}$ $0.1 \ M$ $0.2 \ M$ $1.2 \times 10^{-3}$ $0.2 \ M$ $0.1 \ M$ $2.4 \times 10^{-3}$
For the reaction,the rate of formation of $C$ will be:
| Initial Conc. $(A)$ | Initial Conc. $(B)$ | Initial rate of formation of $C \ (mol \ L^{-1} \ s^{-1})$ |
| $0.1 \ M$ | $0.1 \ M$ | $1.2 \times 10^{-3}$ |
| $0.1 \ M$ | $0.2 \ M$ | $1.2 \times 10^{-3}$ |
| $0.2 \ M$ | $0.1 \ M$ | $2.4 \times 10^{-3}$ |
For the reaction,the rate of formation of $C$ will be:
Medium
View SolutionFor the reaction $2A + 2B \rightarrow 2C + D$,if $r = k[A]^2[B]^0$,then the rate of reaction is:
The acidic hydrolysis of an ester is a .......
Easy
View SolutionConsider the plots,given below,for the reaction $A \rightarrow B + C$. The plots respectively correspond to the reaction order:
Medium
View SolutionRate law for the reaction $aA + bB \rightarrow cC + dD$ is $r = k[A][B]$. The rate of reaction doubles if:
Vedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo